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Canadian
International
Matriculation
Programme
SCH4U CHEMISTRY FINAL EXAMINATION
Date:
Thursday, November 27, 2014
Time:
8:30 AM – 10:30 AM
Length:
2 Hours
Teachers:
Ms. Kimberley Gagnon & Ms. Véronique Turpin
Student Name: ______________________________ Section/Period: _______
INSTRUCTIONS:
1. Circle your teacher’s name above.
2. Write your name, period number and teacher’s name on the Scantron sheet.
3. Check that your examination has 15 typed pages, including the cover page.
4. Answer all questions in the spaces provided.
5. You may use a scientific calculator.
6. Chemistry Periodic Table is attached to the end of the exam. Please tear it off now for
easier referral.
7. There are four parts to the exam. Read instructions to each part carefully.
STRUCTURE/EVALUATION:
PARTS
A
B
C
D
Category
Knowledge and Understanding
Communication
Thinking and Investigation
Application
TOTAL
Mark Distribution
20%, allow 30 minutes
20%, allow 20 minutes
40%, allow 45 minutes
20%, allow 25 minutes
100%, 120 minutes
_________________________________________________________________________
For office use only
24
Part A
Part B
Part C
Part D
Overall
Performance Level
Performance Level
Performance Level
Performance Level
Performance Level
4 3 2 1 R
4 3 2 1 R
4 3 2 1 R
4 3 2 1 R
=4 3 2 1 R
Percentage
______ %
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Part A: Knowledge/Understanding: (allow 30 minutes)
Instructions:
Identify the letter of the choice that best completes the statement, or answers the
question. Shade the correct answer on the scantron sheet provided. Ensure your
name and period number is on this sheet.
Part B: Communication: (allow 20 minutes)
Instructions: Answer all questions in the space provided.
1. Hydrocarbons are compounds which contain carbon and hydrogen atoms. They are insoluble in water,
but are soluble in non-polar solvents. Some examples of hydrocarbons are given below:
The correct order of these hydrocarbons, so that
they represent compounds with triple bond,
double bond, single bond, and those containing
benzene ring respectively, is
_______, _______, _________, and ________.
Explain your reasoning.
Number
1
2
3
4
Name
Alkenes
Alkynes
Alkanes
Aromatic hydrocarbons
2. Draw a Lewis structure for, and indicate the number of sigma and pi bonds in CO2.
3. List the different factors that affect a chemical reaction.
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4. Define percent dissociation of a weak acid.
5. Use oxidation numbers to explain why sulfur acts as a reducing agent in reaction A, but as an oxidizing
agent in reaction B:
Reaction A:
NO3–(aq) + S(s) → SO2(g) + NO(g)
Reaction B:
PO33-(aq) + S(s) → H2S(g) + PO43-(aq)
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Part C: Thinking/Investigation: (allow 45 minutes)
Instructions: Answer six (6) of the following 7 questions ONLY. If you attempt all six CIRCLE the
questions you want marked otherwise the first six will be marked. Write the answer in
the space provided. If the question requires mathematical calculations, show all of
your work. Answer all questions with the correct units and number of significant
figures.
1. Draw and name the products produced in the following diagram.
2. The standard molar enthalpy of formation, ΔHf°, of diborane cannot be determined directly because
the compound cannot be prepared by reaction of boron and hydrogen. However, the value can be
calculated. Calculate the standard enthalpy of formation of gaseous diborane (B2H6) using the
following thermochemical information:
a) 4 B(s) + 3 O2(g) →2 B2O3(s)
ΔH° = -2509.1 kJ
b) 2 H2(g) + O2(g) → 2 H2O(l)
ΔH° = -571.7 kJ
c) B2H6(g) + 3 O2(g) → B2O3(s) + 3 H2O(l) ΔH° = -2147.5 kJ
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3. Lactic acid, CH3CH2OHCO2H, builds up in human muscles during anaerobic exercise. If the initial
concentration of lactic acid is 0.12 mol/L and the pH is 2.39, what is Ka for lactic acid?
4. Balance one of the following redox reactions below:
FeSO4 +
Zn
H2SO4 +
+
NO3-
KMnO4 →
→
Fe2(SO4)3 + K2SO4 + MnSO4 + H2O
ZnO22- +
NH3
in basic conditions
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5. In an electrolysis experiment, silver metal, Ag, is electroplated from a silver nitrate solution by passing
a current of 0.900 A through the cell for 75.0 min. Calculate the mass of silver that is produced. Note:
96 500 C in 1 mole of electrons.
6. Write the ground state electronic configuration for arsenic, As, and then draw the correct energy level
diagram.
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7. For one of the following: HPO42- ion or PCl5 molecule
a. Draw the Lewis structure.
b. Use the VSEPR theory to predict the shape of the compound.
c. State whether the molecule is polar or nonpolar, and draw the dipole moment above for the
molecule if the molecule is polar.
Part D: Application: (allow 25 minutes)
Instructions:
Answer four (4) of the following 5 questions ONLY. If you attempt all five CIRCLE the
questions you want marked otherwise the first four will be marked. If the question
requires mathematical calculations, show all of your work. Answer all questions with
the correct number of significant figures (digits).
1. In the lab, Jamie and Joseph were trying to figure out what organic chemicals were in the five beakers
that they forgot to label on their desk. They then decided to carry out some organic chemistry
reactions to determine what was in them. They were given the following solutions:
hexane, hexene, methylpropanoate, hexanol, and 3-methylhexan-3-ol
They conducted the following tests and obtained the following results: Determine which compound is
which by completing the table.
Tests Conducted
Beaker A
-added KMnO4
Results
-purple solution changed to a
brown precipitate
Beaker B
-added bromine in water
-yellow solution changed to a
colourless solution
Beaker C
-added bromine in water
-placed beaker in the sunlight
-yellow solution changed to a
colourless solution only after it
was placed in the sunlight
Beaker D
- added KMnO4
-purple solution remained
purple
Beaker E
-smelled the solution
-smelled very fruity
Compound
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2. A student heated 200.0g of water with 10.0 g of ethanol, (C2H5OH). What will be the change in the
temperature of the water?
Given:
Q = mc∆T
∆H°comb = -1366.7 kJ/mol
c H2O(l) = 4.19 J/g℃
3. In a closed can of pop, dissolved carbonic acid, H2CO3, is in equilibrium with CO2 and H2O. When the
can is opened, CO2 is produced until the pop goes “flat.” (No more CO2(g) is produced.) Explain these
observations, based on your knowledge of equilibrium and Le Chatelier’s principle.
H2CO3(aq) → CO2(g) + H2O(l)
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4. Can a solution of zinc nitrate be stored in an aluminum container? Explain in terms of the halfreactions, overall reaction, and cell potential involved. The standard reduction potentials for zinc and
aluminum are –0.76 V and –1.66 V, respectively.
5. Choose ONE chemistry related topic from our SCH 4U course and relate it to technology, society and
the environment. Recall our units covered: organic chemistry, structure and matter, rates of reaction,
equilibrium and electrochemistry.
State your topic :
Technology :
Explain the science :
Society :
Environment :
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Periodic Table of the Elements: Tear this page from the exam for easy referral.